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Sponteneous adsorption of a gas on solid surface is an exothermic process because
- a)∆H increases for system
- b)∆S increases for gas
- c)∆S decreases for gas
- d)∆G increases for gas
Correct answer is option 'C'. Can you explain this answer?
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Most Upvoted Answer
Sponteneous adsorption of a gas on solid surface is an exothermic proc...
Explanation:
When a gas spontaneously adsorbs onto a solid surface, it is an exothermic process. This means that heat is released during the adsorption process. The correct answer to the question is option 'C' - the entropy (S) decreases for the gas.
Entropy and Spontaneity:
Entropy is a measure of the disorder or randomness in a system. In a spontaneous process, the entropy of the universe increases. However, when a gas adsorbs onto a solid surface, the gas molecules become more ordered and confined to a smaller space. This leads to a decrease in the entropy of the gas.
Exothermic Process:
An exothermic process is one that releases heat to the surroundings. When a gas adsorbs onto a solid surface, intermolecular forces are formed between the gas molecules and the surface. These forces release energy in the form of heat. Therefore, the process is exothermic.
Explanation of Option 'C':
Option 'C' states that the entropy decreases for the gas. This is the correct answer because when a gas adsorbs onto a solid surface, the gas molecules become more ordered and confined to a smaller space. This decrease in entropy contributes to the exothermic nature of the process.
Explanation of Other Options:
- Option 'A' states that the enthalpy (H) increases for the system. While it is true that heat is released during the adsorption process, the enthalpy change for the system does not necessarily increase. The enthalpy change depends on the specific adsorption process and may be endothermic or exothermic.
- Option 'B' states that the entropy increases for the gas. This is not true because, as mentioned earlier, the gas molecules become more ordered and confined to a smaller space during adsorption, leading to a decrease in entropy.
- Option 'D' states that the Gibbs free energy (G) increases for the gas. The Gibbs free energy change for a process is given by the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change, ΔS is the entropy change, and T is the temperature. Since the process is exothermic (ΔH < 0)="" and="" the="" entropy="" of="" the="" gas="" decreases="" (δs="" />< 0),="" the="" gibbs="" free="" energy="" change="" for="" the="" gas="" is="" likely="" to="" be="" negative="" (δg="" />< 0),="" indicating="" a="" more="" favorable="" and="" spontaneous="" process.="" therefore,="" option="" 'd'="" is="" not="" the="" correct="" answer.="" 0),="" indicating="" a="" more="" favorable="" and="" spontaneous="" process.="" therefore,="" option="" 'd'="" is="" not="" the="" correct="" />
When a gas spontaneously adsorbs onto a solid surface, it is an exothermic process. This means that heat is released during the adsorption process. The correct answer to the question is option 'C' - the entropy (S) decreases for the gas.
Entropy and Spontaneity:
Entropy is a measure of the disorder or randomness in a system. In a spontaneous process, the entropy of the universe increases. However, when a gas adsorbs onto a solid surface, the gas molecules become more ordered and confined to a smaller space. This leads to a decrease in the entropy of the gas.
Exothermic Process:
An exothermic process is one that releases heat to the surroundings. When a gas adsorbs onto a solid surface, intermolecular forces are formed between the gas molecules and the surface. These forces release energy in the form of heat. Therefore, the process is exothermic.
Explanation of Option 'C':
Option 'C' states that the entropy decreases for the gas. This is the correct answer because when a gas adsorbs onto a solid surface, the gas molecules become more ordered and confined to a smaller space. This decrease in entropy contributes to the exothermic nature of the process.
Explanation of Other Options:
- Option 'A' states that the enthalpy (H) increases for the system. While it is true that heat is released during the adsorption process, the enthalpy change for the system does not necessarily increase. The enthalpy change depends on the specific adsorption process and may be endothermic or exothermic.
- Option 'B' states that the entropy increases for the gas. This is not true because, as mentioned earlier, the gas molecules become more ordered and confined to a smaller space during adsorption, leading to a decrease in entropy.
- Option 'D' states that the Gibbs free energy (G) increases for the gas. The Gibbs free energy change for a process is given by the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change, ΔS is the entropy change, and T is the temperature. Since the process is exothermic (ΔH < 0)="" and="" the="" entropy="" of="" the="" gas="" decreases="" (δs="" />< 0),="" the="" gibbs="" free="" energy="" change="" for="" the="" gas="" is="" likely="" to="" be="" negative="" (δg="" />< 0),="" indicating="" a="" more="" favorable="" and="" spontaneous="" process.="" therefore,="" option="" 'd'="" is="" not="" the="" correct="" answer.="" 0),="" indicating="" a="" more="" favorable="" and="" spontaneous="" process.="" therefore,="" option="" 'd'="" is="" not="" the="" correct="" />
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Sponteneous adsorption of a gas on solid surface is an exothermic process becausea)∆H increases for systemb)∆S increases for gasc)∆S decreases for gasd)∆G increases for gasCorrect answer is option 'C'. Can you explain this answer?
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